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Chapter 14

Chapter 14. Liquids and Solids. Comparisons of the States of Matter. the solid and liquid states have a much higher density than the gas state therefore the molar volume of the solid and liquid states is much smaller than the gas state the solid and liquid states have similar densities

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Chapter 14

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  1. Chapter 14 Liquids and Solids

  2. Comparisons of the States of Matter • the solid and liquid states have a much higher density than the gas state • therefore the molar volume of the solid and liquid states is much smaller than the gas state • the solid and liquid states have similar densities • generally the solid state is a little denser • notable exception: ice is less dense than liquid water • the molecules in the solid and liquid state are in close contact with each other, while the molecules in a gas are far apart Tro, Chemistry: A Molecular Approach

  3. Properties of the 3 Phases of Matter • Fixed = keeps shape when placed in a container • Indefinite = takes the shape of the container Tro, Chemistry: A Molecular Approach

  4. Explaining the Properties of Solids • the particles in a solid are packed close together and are fixed in position • though they may vibrate • the close packing of the particles results in solids being incompressible • the inability of the particles to move around results in solids retaining their shape and volume when placed in a new container; and prevents the particles from flowing Tro, Chemistry: A Molecular Approach

  5. Solids • some solids have their particles arranged in an orderly geometric pattern – we call these crystalline solids • salt and diamonds • other solids have particles that do not show a regular geometric pattern over a long range – we call these amorphous solids • plastic and glass Tro, Chemistry: A Molecular Approach

  6. Explaining the Properties of Liquids • they have higher densities than gases because the molecules are in close contact • they have an indefinite shape because the limited freedom of the molecules allows them to move around enough to get to the container walls • but they have a definite volume because the limit on their freedom keeps them from escaping the rest of the molecules Tro, Chemistry: A Molecular Approach

  7. Phase Changes Tro, Chemistry: A Molecular Approach

  8. Energy Requirements for the changes of State • Intramolecular (within the molecule)forces : the bonding forces that hold the atoms of a molecule together • Intermolecular (between molecules) forces : The forces that occurs among molecules that cause them to aggregate to form a solid of a liquid

  9. Energy Requirements for the changes of State • Molar heat of fusion: The energy required to melt 1 mol of a substance • kJ/mol • Molar heat of vaporization: The energy required to change 1 mol of liquid to its vapor • kJ/mol

  10. Calculating Energy Changes: Solid to Liquid and Liquid to Gas • Calculate the energy required to melt 8.5 g of ice at 0.0oC. The molar heat of fusion for ice is 6.02 kJ/mol • Calculate the energy (kJ) required to heat 25 g of liquid water from 25.0oC to 100.0oC and change it to steam at 100.0oC. The specific heat capacity of liquid water is 4.184 J/goC, and the molar heat of vaporization of water is 40.6 kJ/mol • Calculate the energy required to vaporize 35.0 g of water at 100.0oC. The molar heat vaporization of water is 40.6 kJ/mol

  11. Why are molecules attracted to each other? • intermolecular attractions are due to attractive forces between opposite charges • + ion to - ion • + end of polar molecule to - end of polar molecule • H-bonding especially strong • even nonpolar molecules will have temporary charges • larger the charge = stronger attraction • longer the distance = weaker attraction • however, these attractive forces are small relative to the bonding forces between atoms • generally smaller charges • generally over much larger distances Tro, Chemistry: A Molecular Approach

  12. Trends in the Strength of Intermolecular Attraction? • the stronger the attractions between the atoms or molecules, the more energy it will take to separate them • boiling a liquid requires we add enough energy to overcome the attractions between the molecules or atoms • the higher the normal boiling point of the liquid, the stronger the intermolecular attractive forces Tro, Chemistry: A Molecular Approach

  13. + - + - _ + + _ + _ + _ + + + + + + + + + + + + - - - - - - - - - - - - Attractive Forces + - + - Tro, Chemistry: A Molecular Approach

  14. Dispersion Forces • fluctuations in the electron distribution in atoms and molecules result in a temporary dipole • region with excess electron density has partial (─) charge • region with depleted electron density has partial (+) charge • the attractive forces caused by these temporary dipoles are called dispersion forces • aka London Forces • all molecules and atoms will have them • as a temporary dipole is established in one molecule, it induces a dipole in all the surrounding molecules Tro, Chemistry: A Molecular Approach

  15. Dispersion Force Tro, Chemistry: A Molecular Approach

  16. Size of the Induced Dipole • the magnitude of the induced dipole depends on several factors • polarizability of the electrons • volume of the electron cloud • larger molar mass = more electrons = larger electron cloud = increased polarizability = stronger attractions • shape of the molecule • more surface-to-surface contact = larger induced dipole = stronger attraction Tro, Chemistry: A Molecular Approach

  17. Effect of Molecular Sizeon Size of Dispersion Force Noble Gases are all nonpolar atomic elements. As the molar mass increases, the number of electrons increase. Therefore the strength of the dispersion forces increases. The stronger the attractive forces between the molecules, the higher the boiling point will be. Tro, Chemistry: A Molecular Approach

  18. Dipole-Dipole Attractions • polar molecules have a permanent dipole • because of bond polarity and shape • dipole moment • as well as the always present induced dipole • the permanent dipole adds to the attractive forces between the molecules • raising the boiling and melting points relative to nonpolar molecules of similar size and shape Tro, Chemistry: A Molecular Approach

  19. Attractive Forces and Solubility • Solubility depends on the attractive forces of solute and solvent molecules • Like dissolves Like • miscible liquids will always dissolve in each other • polar substance dissolve in polar solvents • hydrophilic groups = OH, CHO, C=O, COOH, NH2, Cl • nonpolar molecules dissolve in nonpolar solvents • hydrophobic groups = C-H, C-C • Many molecules have both hydrophilic and hydrophobic parts - solubility becomes competition between parts Tro, Chemistry: A Molecular Approach

  20. Immiscible Liquids Tro, Chemistry: A Molecular Approach

  21. Dichloromethane (methylene chloride) Ethanol (ethyl alcohol) Water Polar Solvents Tro, Chemistry: A Molecular Approach

  22. Nonpolar Solvents n-hexane toluene carbon tetrachloride Tro, Chemistry: A Molecular Approach

  23. Hydrogen Bonding • When a very electronegative atom is bonded to hydrogen, it strongly pulls the bonding electrons toward it • O-H, N-H, or F-H • Since hydrogen has no other electrons, when it loses the electrons, the nucleus becomes deshielded • exposing the H proton • The exposed proton acts as a very strong center of positive charge, attracting all the electron clouds from neighboring molecules Tro, Chemistry: A Molecular Approach

  24. H-Bonding HF Tro, Chemistry: A Molecular Approach

  25. H-Bonding in Water Tro, Chemistry: A Molecular Approach

  26. Practice – Choose the substance in each pair that is more soluble in water • CH3OH CH3CHF2 • CH3CH2CH2CH3 CH3Cl Tro, Chemistry: A Molecular Approach

  27. Ion-Dipole Attraction • in a mixture, ions from an ionic compound are attracted to the dipole of polar molecules • the strength of the ion-dipole attraction is one of the main factors that determines the solubility of ionic compounds in water Tro, Chemistry: A Molecular Approach

  28. Summary • Dispersion forces are the weakest of the intermolecular attractions. • Dispersion forces are present in all molecules and atoms. • The magnitude of the dispersion forces increases with molar mass • Polar molecules also have dipole-dipole attractive forces Tro, Chemistry: A Molecular Approach

  29. Summary (cont’d) • Hydrogen bonds are the strongest of the intermolecular attractive forces • a pure substance can have • Hydrogen bonds will be present when a molecule has H directly bonded to either O , N, or F atoms • only example of H bonded to F is HF • Ion-dipole attractions are present in mixtures of ionic compounds with polar molecules. • Ion-dipole attractions are the strongest intermolecular attraction • Ion-dipole attractions are especially important in aqueous solutions of ionic compounds Tro, Chemistry: A Molecular Approach

  30. Tro, Chemistry: A Molecular Approach

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